Consider the following reaction: 2 \mathrm{SO}_{3}(\mathrm{~g})<->2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \mathrm{K}_{c}=6.18 In a flask there are 2.10 mol/L of sulfur dioxide gas, 0.10 mol/L of oxygen gas, and 0.32 mol/L of sulfur trioxide

gas. Which way, if at all,will the reaction shift? a. The reaction will shift left to make more reactants. b. The reaction will shift left to make more products. c. The reaction will shift right to make more reactants. d. The reaction is already at equilibrium. The reaction will shift right to make more products.